Maxwell's velocity distribution curve is given for two different temperatures. For the given curves-
                    

1. $T_1>T_2$
2. $T_1<T_2$
3. $T_1\le T_2$
4. $T_1=T_2$

The variation of density (p) of gas with its absolute temperature (T) at constant pressure is best represented by the graph

1.		2.
3.		4.

A gas mixture consists of 2 moles of oxygen and 4 moles of argon at temperature T. Neglecting all vibrational modes, the total internal energy of the system is

1.  4RT

2.  15RT

3.  9RT

4.  11RT

The root mean square speed of oxygen molecules (O2) at a certain absolute temperature is v. If the temperature is doubled and oxygen gas dissociates into oxygen atom, the rms speed would be :

1.  $\mathrm{v}<mspace\; width="1em"></mspace><mspace\; width="1em"></mspace>$

2.  $\sqrt{2}\mathrm{v}<mspace\; width="1em"></mspace><mspace\; width="1em"></mspace>$

3.  $2\mathrm{v}<mspace\; width="1em"></mspace><mspace\; width="1em"></mspace>$

4.  $2\sqrt{2}\mathrm{v}$

The molecules of a given mass of gas have rms velocity of 200 ms^-1 at \(27^{\circ}\mathrm{C}\) and 1.0 x 10⁵ Nm^-2 pressure. When the temperature and pressure of the gas are increased to, respectively, \(127^{\circ}\mathrm{C}\) and 0.05 X 10⁵ Nm^-2, rms velocity of its molecules in ms^-1 will become:
1. 400/√3
2. 100√2/3
3. 100/3 
4.100√2

What is the mass of 2 liters of nitrogen at 22.4 atmospheric pressure and 273 K?

1. 28 g               

2. 14$\times 22.4$ g

3. 56 g               

4. None of these

Gases exert pressure on the walls of containing vessel because  the gas molecules:

1. Possess momentum

2. collide with each other

3. have finite volume

4. obey gas laws

For gas, if the ratio of specific heats at constant pressure p and constant volume V is ${\rm Y}$, then value of degree of freedom is:

1. $\frac{\gamma +1}{\gamma -1}$           

2. $\frac{\gamma -1}{\gamma +1}$           

3. $\frac{\gamma -1}{2}$           

4. $\frac{2}{\gamma -1}$

Four molecules have speeds 2 km/sec, 3 km/sec, 4 km/sec and 5 km/sec.  The root mean square speed of these molecules (km/sec) is:

1. $\sqrt{\frac{54}{4}}$       

2. $\sqrt{\frac{54}{2}}$         

3. 3.5           

4. 3$\sqrt{3}$

One liter of gas A and two liters of gas B, both having the same temperature 100$°$C and the same pressure 2.5 bar will have the ratio of average kinetic energies of their molecules as:

1. 1:1       

2. 1:2     

3. 1:4       

4. 4:1